Question:
What is the oxidation state of Phosphorus in \(H_3PO_4\)?
What is the oxidation state of Phosphorus in \(H_3PO_4\)?
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To find oxidation states quickly, remember common values: Hydrogen \(+1\), Oxygen \(-2\), Alkali metals \(+1\), and the total oxidation number of a neutral compound is always zero.
Updated On: Apr 22, 2026
- \(+3\)
- \(+5\)
- \(+1\)
- \(-3\)
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The Correct Option is B
Solution and Explanation
Concept:
The oxidation state of an element in a compound is calculated by assigning standard oxidation numbers to known atoms and solving for the unknown element. Rules used:
• Hydrogen generally has oxidation state \(+1\)
• Oxygen generally has oxidation state \(-2\)
• The sum of oxidation states in a neutral compound is zero
Step 1: Assign oxidation states to known elements. \[ H = +1, \quad O = -2 \] For \(H_3PO_4\): \[ 3(+1) + x + 4(-2) = 0 \] where \(x\) is the oxidation state of phosphorus.
Step 2: Solve the equation. \[ 3 + x - 8 = 0 \] \[ x - 5 = 0 \] \[ x = +5 \]
Step 3: State the result. \[ \boxed{+5} \]
The oxidation state of an element in a compound is calculated by assigning standard oxidation numbers to known atoms and solving for the unknown element. Rules used:
• Hydrogen generally has oxidation state \(+1\)
• Oxygen generally has oxidation state \(-2\)
• The sum of oxidation states in a neutral compound is zero
Step 1: Assign oxidation states to known elements. \[ H = +1, \quad O = -2 \] For \(H_3PO_4\): \[ 3(+1) + x + 4(-2) = 0 \] where \(x\) is the oxidation state of phosphorus.
Step 2: Solve the equation. \[ 3 + x - 8 = 0 \] \[ x - 5 = 0 \] \[ x = +5 \]
Step 3: State the result. \[ \boxed{+5} \]
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